GCSE Chemistry revision

Metallic bonding

Chemical bonds, ionic, covalent and metallic

AQA 4.2.1.5 Foundation & Higher

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Metals bonding to non-metals form ionic bonds, non-metals bonding to non-metals form covalent bonds, and metals bonding to other metals form metallic bonds.

A solid metal consists of a giant structure of metal atoms arranged in a regular, repeating pattern.
Metal atoms give up their outer shell electrons, becoming positively charged ions within this regular structure.
The released electrons are free to move throughout the entire structure and are called delocalised electrons.

2. Structure of a Metal AQA

A solid metal consists of a giant structure of metal atoms arranged in a regular, repeating pattern.
Metal atoms give up their outer shell electrons, becoming positively charged ions within this regular structure.
The released electrons are free to move throughout the entire structure and are called delocalised electrons.

Metallic bonding is the strong electrostatic attraction between the positive metal ions and the negatively charged delocalised electrons.
These forces of attraction hold the metal ions together in a regular structure, giving the overall metal its strength.

Metals generally have high melting and boiling points, meaning most are solid at room temperature, due to the strong metallic bonds holding the structure together.
Metals are good conductors of electricity because the delocalised electrons can move freely and carry electrical current.
Metals are good conductors of heat because the delocalised electrons can transfer thermal energy through the structure.
Metals are malleable, meaning they can be bent or hammered into shapes, because the regular layers of ions can slide over one another.

4. Properties of Metals Explained AQA

Metals generally have high melting and boiling points, meaning most are solid at room temperature, due to the strong metallic bonds holding the structure together.
Metals are good conductors of electricity because the delocalised electrons can move freely and carry electrical current.
Metals are good conductors of heat because the delocalised electrons can transfer thermal energy through the structure.
Metals are malleable, meaning they can be bent or hammered into shapes, because the regular layers of ions can slide over one another.

An alloy is a mixture containing two or more different elements, typically two different metals or a metal and a non-metal.
Alloys are designed by mixing elements with different sized atoms, which disrupts the regular layered structure of the pure metal.
Because the differently sized atoms prevent the layers from sliding over one another, alloys are much harder than pure metals.

5. What are Alloys? AQA

An alloy is a mixture containing two or more different elements, typically two different metals or a metal and a non-metal.
Alloys are designed by mixing elements with different sized atoms, which disrupts the regular layered structure of the pure metal.
Because the differently sized atoms prevent the layers from sliding over one another, alloys are much harder than pure metals.

Steel is an alloy made mostly of iron with 1–2% carbon added, and sometimes other elements such as chromium, manganese, or vanadium
The addition of carbon and other elements gives steel much greater strength than pure iron, making it suitable for use in cars and planes.